AP Chemistry
7.10 Reaction Quotient and Le Châtelier’s Principle
7.4 Calculating the Equilibrium Constant
7.3 Reaction Quotient and Equilibrium Constant
A reversible reaction is represented by the equation below.
\[ \text{N}_2\text{O}_4(g) \rightleftharpoons 2\,\text{NO}_2(g) \]
At a constant temperature, the system is initially at equilibrium in a \(1.0\text{ L}\) rigid container. At equilibrium, the concentration of \(\text{N}_2\text{O}_4(g)\) is \(0.20\text{ M}\) and the concentration of \(\text{NO}_2(g)\) is \(0.40\text{ M}\). The volume of the container is rapidly expanded to \(2.0\text{ L}\) at the same temperature. What is the value of the reaction quotient, \(Q_c\), immediately after the volume expansion?
\[ \text{N}_2\text{O}_4(g) \rightleftharpoons 2\,\text{NO}_2(g) \]
At a constant temperature, the system is initially at equilibrium in a \(1.0\text{ L}\) rigid container. At equilibrium, the concentration of \(\text{N}_2\text{O}_4(g)\) is \(0.20\text{ M}\) and the concentration of \(\text{NO}_2(g)\) is \(0.40\text{ M}\). The volume of the container is rapidly expanded to \(2.0\text{ L}\) at the same temperature. What is the value of the reaction quotient, \(Q_c\), immediately after the volume expansion?
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